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![3. Give the balanced equation which shows the decomposition reaction of solid aluminum
chlorate [Al(ClO3)3] with heat.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb0fb29b5-807b-4f7b-9db1-fb381e467b35%2F1007853a-336a-4213-8125-6954a4a0a2e9%2Fj3mlr1j_processed.jpeg&w=3840&q=75)
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- What is wrong with the chemical formula [CO(H2O)4SCN]V and what is the right formula and name for it?Given: You weigh out exactly 0.200 g of Fe(NH4)2(SO4)2·6H2O and dissolve it in the 100.00 mL volumetric flask. You then pipette 2.00 mL of this solution into the 50.00 mL volumetric flask to prepare the stock standard tris-bipyridyl-iron(II) solution. a. Calculate the molar concentration of iron(II) in this solution in the 50.00 mL volumetric flask. (The MW of Fe(NH4)2(SO4)2·6H2O is 392.14 g/mol) (answer a given the information above)Chromium metal is obtained by reduction of chromium(III) oxide with powdered aluminum. The reaction is highly exothermic, and the products are molten Al2O3(l) and Cr(l) . Write the balanced equation for this reduction.
- What is the importance and uses of pure cobalt(II) sulphate?Why is the oxidation state of Fe 2.5?The aluminium in a 1.2 g sample of impure NH4Al (SO4)2 was precipitated as hydrous Al2O3. The precipitate was filtered and ignited at 100° c to give anhydrous Al2O3 which weighed 0.1798 g. Calculate the % Al in the sample. (number of moles Al = 2; Al2O3 = 1)
- A 0.8102 g sample of impure Al2(CO3)3 was decomposed with HCl; the liberated CO2 was collected on calcium oxide and found to weigh 0.0515 g. Calculate the percentage of aluminum in the original sample. [Note: Assume all the collected CO2 came from the Al2(CO3)3 and Hint: Write the balanced chemical reaction.]Consider the following equation: CuSO4•5H2O + Fe → FeSO4 + Cu + 5H2O. Which substance is oxidized and which is reduced?What is the net ionic equation of the reaction of FeCl2 with NaOH? what is the net ionic equation of the reaction of MgSO4 with Ba(NaO3)2?
- (b) A metallurgical laboratory carried out analysis of a sample in which analysis of Mn was done by forming a precipitate of MNSO4. If 3.18 g of ore sample gives 0.28 g of MnSO4. Calculate the percentage of Mn [9] present in the sample.The price of (a) CoCl2•6H2O is $25.00 per 100 g and (b) NH,CI was $11.35 per 500 g. Calculate the costs of each of these reagents used in this preparation. If cost were a determining factor which of these would be used as a limiting reagent? (a)One of the steps for refining silver involves converting silver into dicyanoargenate(I) ions: 4Ag(s) + 8CN−(aq) + O2(g) + 2H2O(l) ⟶ 4[Ag(CN)2]−(aq) + 4OH−(aq)Explain why oxygen must be present to carry out the reaction. Why does the reaction not occur as: 4Ag(s) + 8CN−(aq) ⟶ 4[Ag(CN)2−(aq)?